each tablespoon of the liquid contains 95mg of aluminum hydroxide and 412mg of magnesium carbonate.how many moles of hydronium ion can be neutralized by one tablespoon of it?al(oh)3 =78g/mol

;mgCo3 =84.3 g/mol

why it is nesessary to cool down the sample before titration in antacid anlaysis ?

If you take many more chemistry courses you will NOT be able to get away with using lower case for formulas. mgCo3 actually means milligrams carbon + o3 means nothing.

To solve the problem, first write the equations and balance them.
Al(OH)3 + 3H^+ ==> Al^+3 + 3H2O
Mg(OH)2 + 2H^+ ==> Mg^+2 + 2H2O

moles Al(OH)3 in 95 mg = grams/molar mass.
moles Mg(OH)2 in 412 mg = grams/molar mass.

Using the coefficients in the balanced equation, convert moles Al(OH)3 to moles H^+.
Do the same for Mg(OH)2.
Then add moles H^+ from the Al compound to moles H^+ from the Mg compound to arrive at the total moles H^+ neutralized by a table spoon of the stuff.

To determine the number of moles of hydronium ions that can be neutralized by one tablespoon of the given liquid, we need to find out the number of moles of aluminum hydroxide (Al(OH)3) and magnesium carbonate (MgCO3) present in one tablespoon.

First, let's convert the given masses of aluminum hydroxide and magnesium carbonate from milligrams (mg) to grams (g), as the molar masses are given in grams per mole (g/mol):

Aluminum hydroxide (Al(OH)3):
Mass = 95 mg = 95/1000 g = 0.095 g

Magnesium carbonate (MgCO3):
Mass = 412 mg = 412/1000 g = 0.412 g

Next, we calculate the number of moles using the molar masses of aluminum hydroxide and magnesium carbonate:

Molar mass of aluminum hydroxide (Al(OH)3) = 78 g/mol
Moles of aluminum hydroxide = Mass / Molar mass
Moles of aluminum hydroxide = 0.095 g / 78 g/mol = 0.001218 moles

Molar mass of magnesium carbonate (MgCO3) = 84.3 g/mol
Moles of magnesium carbonate = Mass / Molar mass
Moles of magnesium carbonate = 0.412 g / 84.3 g/mol = 0.004884 moles

Since hydronium ions (H3O+) can react with one mole of each aluminum hydroxide and magnesium carbonate, we add the number of moles of aluminum hydroxide and magnesium carbonate to find the total number of moles of hydronium ions that can be neutralized:

Total moles of hydronium ions = Moles of aluminum hydroxide + Moles of magnesium carbonate
Total moles of hydronium ions = 0.001218 moles + 0.004884 moles = 0.006102 moles

Therefore, one tablespoon of the given liquid can neutralize approximately 0.006102 moles of hydronium ions.